Using the table provided, determine which of the following statements is true about the reaction of solid sodium with chlorine gas (2 Na (s) + 1 Cl2 (g) arrow 2 NaCl(s)) at 25 degrees Celsius and 1 atmosphere.
The reaction produces no change in ΔG.
The reaction is nonspontaneous.
The reaction is spontaneous.
The reaction produces a +ΔG.
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Ok thank you
Ok so looking at your table,
Notice two things.
In the equation you have Na and cl2
So notice you have deltaG of formation which, the concept is the same for Hear of formation in the sense that naturally occurring elements have Delta g of formation of 0
So Na and chlorine gas have delta g of formation of 0
You notice that the delta G of formation for NaCl is both large and negative. So it's spontaneous.
Note delta g of formation is for one mole of the substance so in our case we would multiply this value by 2
So it is C?
This kind of makes sense, for multiple reasons. Why it's so large. Technically chlorine wants that electron so badly and sodium wants to lose the electron to
Achieve octet so, once the bond forms you'll release a lot of energy. You'll get a bond that's more like an ionic bond one in which electrons are transfered from Sodium to Cl, in NaCl
Thanks again. I have a couple I am going to post, just to check my answer.